answer

watching

views

20 Jun 2020

Calculate for the , in , of a reaction with a value of if the anode half-cell is saturated with and the cathode half-cell solution is of .

Booster class

General Chemistry 2

Skill

Solve problems involving Ecell as a function of concentrations

answer

watching

217

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

1 Sep 2020

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

The cell potential of the following electrochemical cell depends onthe {\rm pH} of the solution in the anode half-cell:
{Pt}}(s) |{H}}_2 (g,1\;{atm}}) | {H}}^ + (aq,?\;{{M}}) ||{Cu}}^{2+} (aq,1.0\; {M}}) | {{Cu}}(s)}.
What is the pH of the solution if E_{cell} is 370 mV?

1) A constant current of 0.800 A is run through the electrolytic cell in order to produce oxygen (gas) at the anode:

2 H₂O â O₂(g) + 4 e^- + 4 H⁺

The amount (in grams) of O₂ obtained after 15.2 min of electrolysis is [X] g

2) Electrolysis of a solution of Tl³⁺ produces deposition of elemental thallium, Tl, at the cathode. The time (in min.) needed for a constant current of 1.20 A to deposit 0.500 g of Tl(s) is [X] min.

3) An electrochemical cell is described by the following line notation:

Zn(s) Ç Zn²⁺(aq) (0.0420 M) ÇÇ Tl³⁺(aq) (9.06Ã10^-2 M), Tl⁺(aq) (0.0400 M) Ç Pt(s).

Given: EÂ°(Zn²⁺/Zn) = - 0.763 V; EÂ°(Tl³⁺/Tl⁺) = + 1.25 V.

The potential on the cathode half-cell, E₊ = V; the potential on the anode half-cell, E_- = V; and the overall cell potential, E_cell = V.

4) Consider electrolysis of molten copper bromide, CuBr₂. What is the product of this process obtained (a) at the cathode? (b) at the anode?

1. a) Cathode: Cu(s);
(b) Anode: Br₂(l)

2. (a) Cathode: Br₂(l);

(b) Anode: Cu(s)

3. (a) Cathode: Cu²⁺;

(b) Anode: Br^-

4. (a) Cathode: Br^-;

(b) Anode: Cu²⁺

5. (a) Cathode: Cu(s);

(b) Anode: O₂(g)

6. (a) Cathode: H₂(g);

(b) Anode: Cu²⁺

A voltaic cell consists of a copper electrode in a solution of copper(II) ions with unknown concentration, and a palladium electrode in a 0.1 M solution of palladium(II) ions. The palladium electrode is the cathode and its reduction potential is 0.951 V, the Cu electrode is the anode. (7 points)

(a) Write the half-reaction that occurs at the anode and the cathode, as well as the overall cell reaction.

b) What is the concentration of Cu2+ ions in the anode if the cell potential is 0.584 V? What is the error in the Cu2+ concentration if the cell potential measurement has an error of Â±2 mV?

Weekly leaderboard

Home

Homework Help 3,900,000

Chemistry 830,000

Calculate for the , in , of a reaction with a value of if the anode half-cell is saturated with and the cathode half-cell solution is of .

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard